What amount of heat (in kJ) is required to convert 16.6 g of an unknown solid (MM = 67.44 g/mol) at -15.4 °C to a liquid at 42.7 °C? (specific heat capacity of solid = 1.95 J/g･°C; specific

Calculate the amount of energy in kilojoules needed to change 207 g of water ice at –10 °C to steam at 125 ° C. The following constants may be useful: Cm (ice) = 36.57 J mol-1 °C-1 • Cm (water) = 75.40 J mol-1 °C-1 Cm (steam) = 36.04 J mol-1 °C-1 Afus H = +6.01 kJ mol 1 Avap H = +40.67 kJ mol- -1

What amount of heat (in kJ) is required to convert 29.3 g of an unknown solid (MM = 67.44 g/mol) at -15.4 °C to a liquid at 42.7 °C? (heat capacity of solid = 1.95 J/g･°C; heat capacity of liquid = 1.18 J/g･°C; ∆Hfus = 5.72 kJ/mol; Tf = 28.3°C)

What amount of heat (in kJ) is required to convert 15.2 g of an unknown liquid (MM = 67.44 g/mol) at 43.5 °C to a gas at 128.2 °C? (specific heat capacity of liquid = 1.18 J/g･°C; specific heat capacity of gas = 0.792 J/g･°C; ∆Hvap = 30.1 kJ/mol; normal boiling point, Tb = 97.4°C)

What amount of heat (in kJ) is required to convert 26.6 g of an unknown solid (MM = 92.14 g/mol) at -115.0 °C to a liquid at 32.3 °C? (specific heat capacity of solid = 1.06 J/g °C; specific heat capacity of liquid = 1.71 J/g. °C; AHfus = 6.61 kJ/mol; normal freezing point, Tf = -95.0 °C)

15.9 Kj 21.2 kj 48.4 kj 4.04 kj  33.3 kj

How much heat energy is required to convert 40.7 g40.7 g of solid iron at 25 ∘C25 ∘C to liquid iron at 1538 ∘C?1538 ∘C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538 ∘C.1538 ∘C. The specific heat capacity of solid iron is 0.449 J/(g·∘C).

A 0.598 g sample of steam at 107.9 ∘C is condensed into a container with 4.70 g of water at 14.1 ∘C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18  J g⋅ ∘C, the specific heat of steam is 2.01  J g⋅ ∘C, and Δ?vap=40.7 kJ/mol.

Calculate the total amount of energy change for the following heating-cooling curve. The following data for ethyl alcohol, also known as ethanol (C2H5OH), may be of some use: H fusion = 7.61 kJ / molH vaporization = 39.3 kJ / molSpecific heat (C) = 0.97 J / g oC (for solid) Specific heat (C) = 2.46 J / g oC (for liquid) Specific heat (C) = 1.70 J / g oC (for vapor) Melting point = -117.3 oCBoiling point = 78.3 oCCritical temperature = 243 oCCritical pressure = 63.0 atmDensity = 0.789 g / mLTriplepoint=150Kat4.3x10-4 Paq = m C T H = H fusion n H = H vaporization n Draw and label a heating-cooling curve (Temperature vs. Time) for a sample of500.0 mL of ethanol that is cooled from 75.0 oC to -135.0 oC in a closed container at a constant rate. Then calculate H (in kJ) of the process described above. Is this an endothermic or exothermic change?

The enthalpy change for converting 1.00 mol of ice at -50.0 °C to water at 80.0°C is and 1.84 J/g – K, respectively. For H20, A Hfus = 6.01kJ/mol, and AHvap = 40.67 kJ/mol. kJ. The specific heats of ice, water, and steam are 2.09 J/g – K, 4.18 J/g – K, %3D 13.91 12.28 10.15 6.45 7906